sund 1: Η Η Η H—C-C-C-0-H Η Η Η lar orbital type: orbitals in the sigma bond: orbitals in the pi bond: sund 2: Η Η Ο H=C=C= Η Η 0-Η tar orbital type: sigma <> Ο Ο
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
![**Understanding Orbital Overlap in Molecular Bonds**
This section aims to describe the highlighted bonds in terms of the overlap of atomic orbitals for various compounds. Let’s break down each compound.
**(If the highlighted bond is not a pi bond, select the blank option from the dropdown menu.)**
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### Compound 1:
![Chemical structure of Ethanol]
- **Structure Analysis:** In this compound, the highlighted bond is between an oxygen (O) atom and a hydrogen (H) atom.
- **Molecular orbital type:** *Dropdown Menu*
- **Atomic orbitals in the sigma bond:** *Dropdown Menu*
- **Atomic orbitals in the pi bond:** *Dropdown Menu*
Given this bond is typically a single bond, it is a sigma (σ) bond and not a pi (π) bond.
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### Compound 2:
![Chemical structure of Acetic Acid]
- **Structure Analysis:** In this compound, the highlighted bonds are between an oxygen (O) atom and a hydrogen (H) atom, and the double bond between carbon (C) and oxygen (O).
- **Molecular orbital type:** *Dropdown Menu* (Preselected value: sigma)
- **Atomic orbitals in the sigma bond:** *Dropdown Menu* (Preselected value: 1s and sp^3)
- **Atomic orbitals in the pi bond:** *Dropdown Menu*
*Explanation of Diagrams:*
- **Bonding Explanation:** In Compound 2, the highlighted (circled) bond between oxygen and hydrogen is a sigma bond formed by the overlap of a 1s orbital from hydrogen and an sp^3 orbital from oxygen. The other bond (C=O) involves both sigma and pi bonds, with the pi bond involving p orbitals.
**Graphical Representation:**
- **Sigma Bonds:** Represented by the single line connecting two atoms.
- **Pi Bonds:** Represented by a secondary line (or double bond) indicating the additional overlap of unhybridized p orbitals.
This detailed breakdown of bond types and orbital overlaps helps us understand molecular structures and their bonding nature, enhancing our grasp on molecular geometry and chemical bonding.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F44f0cc30-2bd0-44eb-8706-1a92a3cceccd%2F2f3ae605-87b2-4b3d-8ffc-b20cb5ec5b76%2Feu906g_processed.png&w=3840&q=75)
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